Hydrometallurgical process and method for recovering metals

ABSTRACT

A mineral processing facility is provided that includes a cogen plant to provide electrical energy and waste heat to the facility and an electrochemical acid generation plant to generate, from a salt, a mineral acid for use in recovering valuable metals.

CROSS REFERENCE TO RELATED APPLICATION

The present application claims the benefits of U.S. ProvisionalApplication Ser. Nos. 61/297,536, filed Jan. 22, 2010; 61/427,745, filedDec. 28, 2010, and 61/432,075, filed Jan. 12, 2011, all having the sametitle, each of which is incorporated herein by this reference in theirentirety.

FIELD

This disclosure relates generally to mineral processing plants andfacilities and particularly to hydrometallurgical plants and facilitiesfor recovering metals.

BACKGROUND

A common method of recovering valuable metals from ores and concentratesis by leaching with a mineral acid. By way of example, rare earth metalsare generally recovered from bastnaesite by leaching the host rock withhydrochloric acid. Uranium can be recovered from uranium-containing hostrock by leaching with phosphoric acid. Copper, beryllium, nickel, iron,lead, molybdenum, aluminum, and manganese can be recovered from hostrock by leaching with nitric acid. Copper, beryllium, nickel, iron,lead, molybdenum, aluminum, germanium, uranium, gold, silver, cobalt,and manganese can be recovered from host rock by leaching with sulfuricacid or hydrochloric acid.

While leaching is effective in dissolving valuable metals, a number ofobstacles are encountered. Hydrometallurgical processes require water.Water may be available only in limited quantities. The available wateris often saline. Furthermore, any process water generated must besuitable for disposal. Typically, the process water is disposed of usingevaporation ponds, which can be expensive to construct and deleteriousto the environment. Evaporation ponds have particularly long termenvironmental footprints. Furthermore, the leaching process requireselectrical energy. Electrical energy can be difficult or expensive toobtain, particularly when the deposit is in a remote location. Thisgenerally requires the mine operator to construct, at high capital andoperating costs, adequate power generation facilities.

SUMMARY

These and other needs can be addressed by the various aspects,embodiments, and configurations disclosed herein.

In one embodiment, a process is disclosed for recovering a valuablemetal from a valuable metal-containing material using a mineral acidproduced by an electrochemical acid generation process, such as achloralkali cell or bipolar membrane electrodialysis system.

In one configuration, the process includes the steps:

(a) contacting a valuable metal-containing material with a leachingsolution to form a pregnant leach solution comprising a dissolvedvaluable metal;

(b) recovering the dissolved valuable metal to form a valuable metalproduct and a byproduct salt solution, wherein typically at least mostof the byproduct salt solution is derived from a reaction of an acidwith a base in one or both of the contacting and recovering steps;

(c) converting, by one or more of a chloralkali and bipolar membraneelectrodialysis cell, the byproduct salt solution into the acid andbase; and

(d) recycling at least most of the acid and base to the contactingand/or recovering steps.

Commonly, at least most of the byproduct salt solution is converted intoacid and base, and at least most of the acid and base are recycled.

In one application, the acid is a component of the leaching solution,the valuable metal is a rare earth, the acid component is hydrochloricacid, the salt in the byproduct salt solution is one or more of sodiumchloride and potassium chloride, the base is one or more of sodiumhydroxide and potassium hydroxide, and the valuable metal product is arare earth oxide.

In another application, the acid is a component of the leachingsolution, the bipolar membrane electrodialysis cell is employed, thevaluable metal is one or more of copper, beryllium, nickel, iron, lead,molybdenum, and manganese, the acid component is nitric acid, the saltin the byproduct salt solution is one or more of sodium nitrate andpotassium nitrate, and the base is one or more of sodium and potassiumhydroxide.

In another application, the acid is a component of the leachingsolution, the bipolar membrane electrodialysis cell is employed, thevaluable metal is uranium, the acid component is phosphoric acid, thesalt in the byproduct salt solution is one or more of sodium phosphateand potassium phosphate, and the base is one or more of sodium andpotassium hydroxide.

In yet another application, the acid is a component of the leachingsolution, the bipolar membrane electrodialysis cell is employed, thevaluable metal is one or more of a platinum group metal, copper,beryllium, nickel, iron, lead, molybdenum, aluminum, germanium, uranium,gold, silver, cobalt, zinc, cobalt, tin, titanium, chromium, andmanganese, the salt in the byproduct salt solution is one or more ofsodium sulfate and potassium sulfate, the acid component is(hydro)sulfuric acid, and the base is one or more of sodium andpotassium hydroxide.

In yet another application, the acid is a component of the leachingsolution, the valuable metal is one or more of yttrium, scandium, alanthanide, a platinum group metal, copper, chromium, beryllium, nickel,iron, lead, molybdenum, aluminum, germanium, uranium, gold, silver,cobalt, zinc, cobalt, tin, titanium, and manganese, the salt in thebyproduct salt solution is one or more of sodium chloride and potassiumchloride, the acid component is hydrochloric acid, and the base is oneor more of sodium and potassium hydroxide.

The process configuration(s) can include purification of the byproductsalt solution upstream of the electrochemical acid generation plant. Inone example, at least most of a selected polyvalent impurity is removedfrom the byproduct salt solution to form a purified salt solution. Theselected polyvalent impurity is commonly a cation that is removed fromthe byproduct salt solution by precipitation induced by a pH change fromcontact of the base with the byproduct salt solution. In anotherexample, the impurity to be removed is an organic, which may originatein the feed material and/or result from the use of organic reagents inthe process.

The process configuration(s) can also include concentration of thepurified salt solution by a salt concentrator to form a concentrated andpurified salt solution followed by introduction of the concentrated andpurified solution and, optionally a mineral acid, into an anolyterecirculation tank. The salt solution is withdrawn from the tank andprovided to the electrochemical acid generation plant.

To produce hydrochloric acid efficiently, an approximate stoichiometricbalance is typically maintained between chlorine and hydrogen gasproduced in the converting step.

The process is particularly applicable to a metal recovery operation inwhich an acid and base are reacted to produce a salt byproduct solution.The salt byproduct solution is regenerated electrochemically to the acidand base components, which are then reused in the process.

In another embodiment, a cogen plant is used to provide waste heat andelectrical energy to the appropriate process steps in a metal recoveryprocess.

The embodiments, aspects, and configurations can provide a number ofadvantages depending on the particular configuration. First, the processcan be used to dispose economically of waste brine solutions fromterrestrial acquifers and/or generated by industrial processes. Theelectrochemical acid generation plant converts waste salt (e.g., sodiumchloride) water, such as from evaporation ponds and terrestrialacquifers, to a mineral acid (e.g., hydrochloric acid) and othervaluable products, such as sodium hydroxide and sodium hypochlorite. Themineral acid and other valuable products can be used in the industrialprocess (e.g., hydrometallurgical valuable metal recovery process)and/or sold. The material recycle can reduce greatly acid and causticreagent requirements. The cogen plant can provide power and heat to theacid generation plant. This combination can create a positiveenvironmental impact. In one example, 936,000 lb/year of water and104,000,000 lb of salt are recycled back to a mineral processing plant.This methodology can avoid the need for waste water ponds that representlong term environmental footprints while reducing operating costs. Forexample, reagent costs and haulage requirements can be reducedsignificantly. Because the water is internally recycled, the need forfresh water can be reduced dramatically.

These and other advantages will be apparent from this disclosure.

As used herein, “at least one”, “one or more”, and “and/or” areopen-ended expressions that are both conjunctive and disjunctive inoperation. For example, each of the expressions “at least one of A, Band C”, “at least one of A, B, or C”, “one or more of A, B, and C”, “oneor more of A, B, or C” and “A, B, and/or C” means A alone, B alone, Calone, A and B together, A and C together, B and C together, or A, B andC together.

The term “a” or “an” entity refers to one or more of that entity. Assuch, the terms “a” (or “an”), “one or more” and “at least one” can beused interchangeably herein. The terms “comprising”, “including”, and“having” can be used interchangeably.

“Absorption” is the incorporation of a substance in one state intoanother of a different state (e.g. liquids being absorbed by a solid orgases being absorbed by a liquid). Absorption is a physical or chemicalphenomenon or a process in which atoms, molecules, or ions enter somebulk phase—gas, liquid or solid material. This is a different processfrom adsorption, since molecules undergoing absorption are taken up bythe volume, not by the surface (as in the case for adsorption).

“Adsorption” is the adhesion of atoms, ions, biomolecules, or moleculesof gas, liquid, or dissolved solids to a surface. This process creates afilm of the adsorbate (the molecules or atoms being accumulated) on thesurface of the adsorbent. It differs from absorption, in which a fluidpermeates or is dissolved by a liquid or solid. Similar to surfacetension, adsorption is generally a consequence of surface energy. Theexact nature of the bonding depends on the details of the speciesinvolved, but the adsorption process is generally classified asphysisorption (characteristic of weak van der Waals forces)) orchemisorption (characteristic of covalent bonding). It may also occurdue to electrostatic attraction.

A “mill” refers to any facility or set of facilities that process ametal-containing material, typically by recovering, or substantiallyisolating, a metal or metal-containing mineral from a feed material.Generally, the mill includes an open or closed comminution circuit,which includes crushers or autogenous, semi-autogenous, ornon-autogenous grinding mills.

A “mineral acid” is an inorganic acid, such as sulfuric acid, nitricacid, or hydrochloric acid.

A “rare earth” refers to any of a large class of chemical elements,including scandium (atomic number 21), yttrium (39), and the 15 elementsfrom 57 (lanthanum) to 71 (lutetium) (known as the lanthanides).

A “salt” is an ionic compound that results from the neutralizationreaction of an acid and a base. Salts are composed of cations(positively charged ions) and anions (negative ions) so that the productis electrically neutral (without a net charge). These component ions canbe inorganic such as chloride (Cl⁻), as well as organic such as acetate(CH₃COO⁻) and monatomic ions such as fluoride (F⁻), as well aspolyatomic ions such as sulfate (SO₄ ² ⁻). Salts that hydrolyze toproduce hydroxide ions when dissolved in water are basic salts and saltsthat hydrolyze to produce hydronium ions in water are acid salts.Neutral salts are those that are neither acid nor basic salts.

A “sorbent” is a material that sorbs another substance; that is, thematerial has the capacity or tendency to take it up by sorption.

“Sorb” means to take up a liquid or a gas either by sorption.

“Sorption” refers to adsorption and absorption, while desorption is thereverse of adsorption.

The preceding is a simplified summary to provide an understanding ofsome aspects of the aspects, embodiments and configurations disclosedherein. This summary is neither an extensive nor exhaustive overview ofthe aspects, embodiments, or configurations. It is intended neither toidentify key or critical elements nor to delineate the scope of theaspects, embodiments, or configurations but to present selected conceptsin a simplified form as an introduction to the more detailed descriptionpresented below. As will be appreciated, other aspects, embodiments, andconfigurations are possible utilizing, alone or in combination, one ormore of the features set forth above or described in detail below.

BRIEF DESCRIPTION OF THE DRAWINGS

The accompanying drawings are incorporated into and form a part of thespecification to illustrate examples of the aspects, embodiments, orconfigurations disclosed herein. These drawings together with thedescription, explain the principle of the aspects, embodiments, orconfigurations. The drawings simply illustrate preferred and alternativeexamples of how the aspects, embodiments, or configurations can be madeand used and are not to be construed as limiting the aspects,embodiments, or configurations to only the illustrated and describedexamples. Further features and advantages will become apparent from thefollowing, more detailed, description of the various aspects,embodiments, or configurations, as illustrated by the drawingsreferenced below.

FIG. 1 is a block diagram depicting a plant according to an embodiment;

FIG. 2 is a block diagram depicting a plant according to an embodiment;

FIG. 3 is a block diagram depicting a purification process according toan embodiment;

FIG. 4 shows the concentration of each of divalent magnesium, calcium,strontium and barium cations in the feed solution and after each of theprecipitation stages M1, M2, M3 and ion exchange stages IX1 and IX2;

FIG. 5 shows the concentration of each of trivalent lanthanum, cerium,praseodymium, neodymium, samarium and iron cations in the feed solutionand after each of the precipitation stages M1, M2, M3 and ion exchangestages IX1 and IX2;

FIG. 6 shows challenge curve for Amberlite 748i (about 4 grams)challenged with a solution containing about 83 mg of lanthanum/L (aslanthanum chloride) at a flow rate of about 2.5 mL/minute at about 21degrees Celsius, with the x-axis being the total volume of lanthanumsolution challenging the Amberlite 748i and the y-axis being thelanthanum concentration in mg/L of the effluent from the challengedcolumn;

FIG. 7 shows concentration of lanthan contained within each fractioncollected from an Amberlite 748i resin loaded with lanthanum;

FIG. 8 shows concentration of lanthanum contained with each fractioncollected from an Amberlite resin IPC 747 resin loaded with lanthanum;

FIG. 9 shows the variation of current, voltage, temperature and salinityduring a salt splitting process for 12 L of a 75 g NaCl/liter solution;and

FIG. 10 shows, as a function of time, the current, voltage andtemperature of a salt splitting process for a salt feed having 95 gNaCl/L and the resulting decrease in of NaCl concentration for the saltfeed and the respective increases in the acid and base concentrations inacid and base tanks of the salt splitting cell.

DETAILED DESCRIPTION

A first embodiment is an industrial plant 100 for processing a feedmaterial 104. The industrial plant 100 first will be discussed withreference to FIG. 1. The industrial plant 100 includes a mill 108, aprocess plant 112, an electrochemical acid generation plant 116, and acogen plant 120. The industrial plant 100 processes a valuablemetal-containing feed material 104.

The valuable metal-containing feed material 104 may comprise a minedore, concentrate, tailings, metallurgical residue or a mixture thereof.Commonly, the valuable metal-containing feed material 104 comprises anacid soluble metal. Referring to the Periodic Table of the Elements, thevaluable metal is typically a transition metal, other metal, actinidemetal, or rare earth metal (e.g., lanthanide). The metal may qualify asa light or heavy metal. Specific examples of valuable metals includeantimony, uranium, lanthanides, copper, beryllium, nickel, iron, lead,molybdenum, aluminum, germanium, uranium, titanium, chromium, gold,silver, cobalt, tin, zinc, cadmium, manganese, and the platinum groupmetals. The metal in the valuable metal-containing material 104 istypically in the form of an igneous (whether abyssal, plutonic,hypabyssal, or extrusive or effusive), metamorphic (whether of ignous orsedimentary origin), or sedimentary (whether clastic sediments orchemical precipitates) mineral, such as a sulfide, oxide, phosphate,carbonate, halide, sulfate, silicate, telluride, oxysalt, sulfosalt, andmixtures thereof. Exemplary rare earth-containing minerals includebastnaesite (a carbonate-fluoride mineral) and monazite. Other rareearth-containing minerals include aeschynite, allanite, apatite,britholite, brockite, cerite, fluorcerite, fluorite, gadolinite,parisite, stillwellite, synchisite, titanite, xenotime, zircon, andzirconolite. Exemplary uranium minerals include uraninite (UO₂),pitchblende (a mixed oxide, usually U₃ O₈), brannerite (a complex oxideof uranium, rare-earths, iron and titanium), coffinite (uraniumsilicate), carnotite, autunite, davidite, gummite, torbernite anduranophane. Exemplary copper minerals include cuprite, chalcolate,covelite, bornite, malachite, azurite, chryscolla, and chalcopyrite.Exemplary nickel minerals include millerite and smaltite. Exemplarycobalt minerals include arsenide Co(As₂), known as smaltite or speisscobalt; cobalt sulfarsenide (CoAsS), known as cobaltite or cobaltglance; and hydrated arsenate (Co(AsO₄)₂.8H₂O), known as erythrite orcobalt bloom. Exemplary molybdenum minerals include molybdenite (MoS₂)and wulfenite (PbMoO₄). As will be appreciated and noted above, valuablemetals are included in a large variety of other minerals known to thoseof skill in the art. As will be further appreciated, the valuablemetal-containing feed material 104 may include a mixture of minerals ofdifferent metals and/or a mixture of valuable metal-containing minerals,invaluable metal-containing minerals, and/or nonmetal-containingminerals.

The valuable metal-containing feed material 104 is introduced into themill 108 to produce a milled material 122 and waste material 124.Depending on the valuable metal-containing feed material 104, the mill108 may have any of a number of differing configurations.

In one configuration, the mill 108 includes a wet (using water 128)and/or dry comminution circuit to reduce an average or median size ofthe incoming valuable metal-containing feed material 104, one or moreconditioning vessels to condition the comminuted feed material forsubsequent processing, and a direct or reverse flotation circuit toisolate in a concentrate or tailings fraction, respectively, themetal-containing mineral(s). The flotation circuit may operate at anelevated temperature (relative to the ambient temperature and/ortemperature of the comminuted feed material). The mill 108 can have, orinclude, other concentration devices or mechanisms, such as gravity orspecific gravity separation mechanisms (e.g., decantation circuits,cyclones, hydraulic classifiers, mechanical classifiers, settling tanks,and the like), size separation mechanisms (e.g., stationary andvibrating screens, filters, grizzlies, trommels, and the like), magneticseparation mechanisms, and color separation mechanisms. The mill 108 caninclude other components, including dryers, slurry vessels, mixing orconditioning vessels, pumps, thickeners, conveyors, screw feeders,agitators, and the like. Water 128 is used to slurry the feed materialfor subsequent processing.

The process plant 112 converts the milled material 122 into ametal-containing product 136 and a byproduct or waste product 132.Depending on the milled material 122, the process plant 112, like themill 108, can have any of a number of differing configurations.

In one configuration, the process plant 112 includes an oxidative ornon-oxidative leaching circuit, which may be an atmospheric orsuper-atmospheric heap, vat, and/or tank leach, conducted at an ambientor elevated temperature, in which a lixiviant is applied to the milledmaterial 122 to leach and/or dissolve, chemically and/or biologically,at least most of one or more of the valuable metals from the milledmaterial 122, leaving behind the byproduct and/or waste 132. Thebyproduct material 132 may comprise a barren valuable metal-containingmaterial. The lixiviant may, or alternatively, also be used to overcomethe inhibitory effect of sulfides, carbonates, oxides, phosphates,halides, silicates, and the like contained with some valuablemetal-containing materials 104.

The composition of the lixiviant depends on the composition of thevaluable metal-containing material 104. Typical lixiviants are mineralacids, such as sulfuric acid, nitric acid, phosphoric acid, hydrobromicacid, hydrochloric acid, hydroiodic acid, hydrofluoric acid, andmixtures thereof. The lixiviant may include other inorganic and organicacids. Once dissolved, the valuable metal is isolated from impurities,such iron, by a suitable recovery technique, such as precipitation,(cationic and/or anionic) ion exchange (e.g., by a resin or solvent),sorption (e.g., carbon-in-leach and resin-in-leach), solvent extraction,electrochemistry (e.g., electrowinning), calcination, roasting,smelting, amalgamation, cementation, gravimetry, other types ofrefining, and combinations thereof. The process plant 112 may includeother components, including dryers, slurry vessels, mixing vessels,conditioning vessels, pumps, thickeners, conveyors, filters, screwfeeders, agitators, and the like. As will be appreciated, mineral acidsand salts can also be used to as a stripping agent for removing avaluable metal from an ion exchange media (e.g., resins or solvent) or asorbent and/or as an electrolyte in electrowinning.

In one configuration of the process plant 112, caustic soda (NaOH) isused in solvent extraction to provide sodium ions to the ion exchangeresin. Rare earth metal ions replace the sodium ions on the ion exchangeresin. The rare earth metal ions are stripped from the resin byhydrochloric acid for subsequent recovery by techniques known to thoseof skill in the art of extractive metallurgy.

The industrial plant 100 further includes the electrochemical acidgeneration plant 116. Commonly, the electrochemical acid generationplant 116 produces from a salt 118 at least most of one or more of thelixiviant, stripping agent and/or electrolyte used by the process plant112. The electrochemical acid generation plant 116 electrolyzes ahalogen-containing alkali metal salt to produce an elemental form of thehalogen and an alkali metal hydroxide. The electrochemical acidgeneration plant 116 can have differing configurations and commonlyincludes one of a chloralkali electrolysis process, a salt splittingelectrolytic process or an bipolar membrane electrodialysis process, ora combination thereof.

As will be appreciated, the chloralkali process can be configured as amembrane electrolysis cell, diaphragm electrolysis cell, or mercury(e.g., Castner-Kellner process) electrolysis cell. Because ofenvironmental problems associated with mercury, the preferred cell typeis the membrane cell.

In the membrane cell, the chloralkali process electrolyzes, in theanodic compartment, a saturated or substantially saturatedhalogen-containing (commonly alkali metal-containing) salt (e.g., achlorine containing salt) to produce an elemental form of the halogen(e.g., chlorine gas) and a salt cation (e.g., alkali-metal) hydroxide.Commonly, the hydroxide comprises caustic soda, (e.g., sodiumhydroxide). An anode and cathode are electrically interconnected and anelectric potential is applied to the anode and cathode by the cogenplant 120 and electric current flows between the anode and cathode. Atthe anode, chloride ions are oxidized to chlorine:

2Cl⁻→Cl₂+2e⁻  (1)

At the cathode, hydrogen in the water is reduced to hydrogen gas,releasing hydroxide ions to the solution:

2H₂O+2e⁻→H₂+2OH⁻  (2)

The chloralkali process includes an ion permeable membrane separatingthe anodic and cathodic compartments. To maintain charge balance betweenthe anodic and cathodic compartments, the cations (e.g., Na⁺or K⁺) passfrom anodic compartment through the ion permeable membrane to thecathodic compartment, where they react with hydroxide ions to produce,for example, caustic soda (NaOH). At least most of the halogen anions(such as chloride anions) and other anions (such as hydroxide ions) arenot passed by the membrane and maintained within the anodic compartment.Assuming that the brine is NaCl, the overall reaction for theelectrolysis of the brine is thus:

2NaCl+2H₂O→Cl₂+H₂+2NaOH  (3)

In the case of potassium chloride as the salt 118, electrolysis of thesalt produces chlorine gas in the anodic compartment and potassiumhydroxide in the cathodic compartment.

The membrane prevents reaction between the chlorine and hydroxide ions.If the reaction were to occur, the chlorine would be disproportionatedto form chloride and hypochlorite ions:

Cl₂+2OH⁻→Cl⁻+ClO⁻+2H₂O  (4)

Above about 60° C., chlorate can be formed:

3Cl₂+6OH⁻→5Cl⁻+ClO₃ ⁻+3H₂O  (5)

If the chlorine gas produced at the anode and sodium hydroxide producedat the cathode were to be combined, sodium hypochlorite (NaClO) (seeequation 6 below) and/or sodium chlorate (NaClO₃) would be produced.

In the diaphragm cell, anodic and cathodic compartments are separated byan ion permeable diaphragm. Brine is introduced into the anodecompartment and flows into the cathode compartment. Like the membranecell, halogen ions are oxidized at the anode to produce elementalhalogens, and, at the cathode, water is split, for example, into causticsoda and hydrogen. The diaphragm prevents the reaction of the causticsoda with the halogen. A diluted caustic brine leaves the cell. Thecaustic soda typically is concentrated to about 50%, and the salt isremoved. This can be done using an evaporative process (discussedbelow). The halogen commonly contains molecular oxygen that can beremoved by liquefaction and evaporation.

The ion-exchange membrane can be any cation- or anion-ion permeablemembrane or bipolar membrane, commonly an ion membrane substantiallystable in the presence of hydroxide anions. More commonly, the ionmembrane is permeable to alkali ions and substantially impermeable tohydroxide and/or halide anions. The ion permeable membrane can comprisea fluoropolymer having one or more pendant sulfonic acid groups, acomposite of fluoropolymers having one or more sulfonic acid groups, anda fluoropolymer having one or more carboxylic acid groups, phosphoricacid groups, and/or a sulfonamide groups and fluorinated membranes. Anexemplary membrane is Nafion™ produced by DuPont, which passessubstantially cations but substantially repels neutrals and anions.

The diaphragm can be any suitable ion permeable material. Typically, thediaphragm is an ion permeable membrane made from asbestos.

It can be appreciated that, while the chloralkali process has beendiscussed in terms of alkali cations, having a +1 charge, the processcan include cations other than alkali cations. The other cations canhave a +2, +3 or +4 charge. The ionic membrane can be configured to bepermeable to the other cations and/or to pass cations having a selectedionic and/or hydrodynamic radius.

A number of products can be formed. Using sodium chloride as anexemplary brine solution:

Cl₂+2NaOH→2NaClO_((bleach))  (6)

Cl₂+H₂→2HCl_((g))  (7)

HCl_((g))+H₂O→HCl_((aq))  (8)

Equation 7 is catalyzed by an alkaline earth metal, typically calcium.

These equations apply to KCl as the salt, if K is substituted for Na.

These equations also apply to halogens other than chlorine providedsuitable changes are made for differences in oxidation states.

In another embodiment, the ionic membrane can comprise an bipolarmembrane electrodialysis membrane process. Commonly, the bipolarmembrane electrodialysis process is conducted in an bipolar membraneelectrodialysis cell having a feed (diluate) compartment, such as thecathodic compartment, and a concentrate (brine) compartment, such as theanodic compartment, separated by one or more anion exchange membranesand one or more cation exchange membranes placed between the anodic anda cathodic compartments. In most bipolar membrane electrodialysisprocesses, multiple bipolar membrane electrodialysis cells are arrangedinto a configuration called an bipolar membrane electrodialysis stack,with alternating anion and cation exchange membranes forming themultiple bipolar membrane electrodialysis stacks. Bipolar membraneelectrodialysis processes are unique compared to distillation techniquesand other membrane-based processes (such as reverse osmosis) in thatdissolved species are moved away from the feed stream rather than thereverse.

A bipolar membrane electrodialysis, or “water splitting”, process,converts aqueous salt solutions into acids and bases, typically withoutchemical addition, avoiding by-product or waste streams and costlydownstream purification steps. Under the force of an electrical field, abipolar membrane can dissociate water into hydrogen (H+, in fact“hydronium” H3O+) and hydroxyl (OH−) ions. The membrane is formed ofanion- and cation-exchange layers and a thin interface where the waterdiffuses from outside aqueous salt solutions. The transport, out of thebipolar membrane, of the H+ and OH− ions obtained from the watersplitting reaction is possible if the bipolar membrane is electricallyoriented correctly. With the anion-exchange side facing the anode andthe cation-exchange side facing the cathode, the hydroxyl anions aretransported across the anion-exchange layer and the hydrogen cationsacross the cation-exchange layer. The generated hydroxyl and hydrogenions are used in an electrodialysis stack to combine with the cationsand anions of the salt to produce acids and bases.

Bipolar membrane electrolydialysis can use many different cellconfigurations. For example, a three-compartment cell is formed bylocating the bipolar membrane in a conventional electrodialysis cell.The bipolar membrane is flanked on either side by the anion- andcation-exchange membranes to form three compartments, namely acidbetween the bipolar and the anion-exchange membranes, base between thebipolar and the cation-exchange membranes, and salt between the cation-and anion-exchange membranes. As in electrodialysis stacks, many cellscan be installed in one stack and a system of manifolds feeds all thecorresponding compartments in parallel, creating three circuits acrossthe stack: acid, base, and salt. Other configurations includetwo-compartment cells with bipolar and cation-exchange membranes (only)or with bipolar and anion-exchange membranes.

As will be appreciated, the electrochemical acid generation plant 116can include an bipolar membrane electrodialysis process conducted priorto and/or after the chloralkali process. The bipolar membraneelectrodialysis process further purifies the aqueous streams produced bythe respective anodic and cathodic compartments.

Commonly at least most of the mineral acid 142 and hydroxide 190 used inthe process plant, such as for a lixiviant, stripping or regenerationagent, or electrolyte, is produced by the electrochemical acidgeneration plant 116 from a suitable salt. By way of example,hydrochloric acid is produced from an alkali metal chloride by burningchlorine gas from the anode compartment and hydrogen gas from thecathode compartment, typically in the presence of a suitable catalyst(see equation 7 above). Hydrosulfuric or sulfuric acid is produced,using salt splitting or bipolar membrane electrodialysis techniques,from an alkali metal sulfate. In other examples, nitric acid is producedfrom an alkali metal nitrate, phosphoric acid is produced from an akalimetal phosphate, hydrobromic acid from alkali metal bromides, hydroiodicacid from alkali metal iodides, and hydrofluoric acid from alkali metalfluorides.

The electrochemical acid generation plant 116 can also produce products140 for sale and water 198 for recycle. Examples of such productsinclude hydrogen gas, a halogen gas (such as chlorine gas, bromine gas,iodine gas, and the like), caustic soda, bleach (such as hypochlorite)and the like.

In one configuration, the salt-containing solution 150 is outputted bythe process plant 112. The salt-containing solution 150 can, forexample, be produced by one or more of the leaching, solvent extractionand electrowinning process(es). In one process plant configuration 12,caustic soda is used in solvent extraction to provide sodium ions to theion exchange resin. Valuable metal ions replace the sodium ions on theion exchange resin. The valuable metal ions are stripped from the resinby hydrochloric acid for subsequent recovery by techniques known tothose of skill in the art of extractive metallurgy.

In the electrochemical acid generation plant, the salt-containingsolution 150 is subjected to chemical treatment, in a primarypurification system, using caustic soda (or cell liquor from the cathodecompartment of the plant 116), sodium carbonate, and/or other additivesthat eliminate at least most of any polyvalent metal ion impurities,such as calcium, magnesium, and iron. Such polyvalent cations candetrimentally impact the performance and operational life of the ionexchange membrane and/or bipolar membrane electrodialysis stack. One orboth of a thickener and filter commonly remove the polyvalentimpurities.

The treated salt-containing solution is then passed through a secondarypurification system to remove most of any remaining polyvalent cations.Caustic soda may be used to adjust the pH to above about pH 7 prior tointroduction into the secondary purification system. Any conventionalsecondary brine purification treatment system associated with membraneoperations may be used, such as a chelating ion exchange resin.Phosphate treatment of the brine may also be used. Phosphates can form agel coat in the membrane in a way that better maintains membraneefficiency. The purified salt-containing solution is then processed by asalt concentrator, such as an evaporator, energy efficient vaporrecompressor, or combination thereof. Proper design of these units withproper use of heat recuperators and elutriation legs has been determinedto be energy efficient and the required slurry concentrations easy tocontrol without the need to centrifuge and separate the solid salt fromthe slurry. The slurry is then introduced into an anolyte recirculationtank, to which a mineral acid, such as hydrochloric acid (produced fromchlorine and hydrogen gases), can be introduced. From the anolyterecirculation tank, the slurry is introduced into the anode compartment.This process is not required where the chloralkali cell uses a diaphragmrather than a membrane.

Turning now to the cogen plant 120, the cogen plant 120 uses anysuitable fuel source 160 to generate power 170 and waste heat 180 (e.g.,steam). The power 170 is used in unit operations in one or more of themill 108, process plant 112, and electrochemical acid generation plant116. As will be appreciated, “cogen” or cogeneration uses a heat engineor a power station to simultaneously generate both electricity anduseful heat. Although any cogeneration plant may be used, common cogenplants include gas turbine cogen plants using the waste heat in the fluegas of gas turbines, gas engine cogen plants using a reciprocating gasengine, combined cycle power plants adapted for cogeneration, steamturbine cogen plants using the heating system as the steam condenser forthe steam turbine, and molten-carbonate fuel cells having a hot exhaustthat is suitable for heating. Smaller cogen plants typically use areciprocating or Stirling engine. The heat is removed from the exhaustand the radiator.

The fuel source 160 can be any suitable combustion fuel source,including compressed or liquefied natural gas, coal, methane, petroleum,liquefied petroleum gas, diesel fuel, kerosene, coal, propane, otherfossil fuels, radioactive materials (e.g., uranium), and alternativefuel sources, such as biodiesel, bioalcohol (methanol, ethanol, andbutanol), hydrogen, HCNG, liquid nitrogen, compressed air, non-fossilmethane, non-fossil natural gas, vegetable oil, and biomass sources.

The waste heat 180 can be directly provided to one or more of the unitoperations, such as flotation, leaching, and the like, by means of aheat exchange loop, which circulates the waste heat 180 from the cogenplant 120 through a heat exchange loop in thermal contact with thematerial in the unit operation to be heated. Alternatively, anintermediate heat exchange medium can collect the waste heat 180, bymeans of a first heat exchange loop, from the waste heat 180 and providethe thermal energy to the material to be heated by means of a secondheat exchange loop.

The operation of the industrial plant 100 will now be discussed withrespect to several illustrative embodiments.

With reference to FIG. 1, the valuable metal-containing feed material104 is introduced into the mill 108 to yield a milled material 122. Inone process configuration, the feed material 104 comprises one or morerare earth-containing minerals, which are crushed and ground. The groundmaterial is subjected to direct flotation, at elevated temperature(which can be in the range of about 30 to about 70° C.) and usingsuitable frothers, collectors, activators, and/or depressants known tothose of ordinary skill in the art, to produce a concentrate (or milledmaterial 120) comprising at least most of the rare earth minerals andtailings. The tailings are commonly suitable for disposal andsubstantially depleted of the rare earths.

The cogen plant 120 provides power to the comminution and flotation cellagitators and waste heat 180, typically in the form of steam, to theslurried milled material prior to the flotation operation.

The milled material 122, or concentrate fraction, is provided to theprocess plant 112 for further processing.

In a common process configuration for valuable metal recovery, milledmaterial 122 is subjected to vat or heap leaching by a mineral acid,commonly by an aqueous hydrochloric acid solution, to dissolve thevaluable metal and form a pregnant leach solution comprising most of thevaluable metal in the concentrate fraction. The pregnant leach solutionis subjected to solvent extraction or ion exchange to remove at leastmost of the dissolved valuable metal from the solution and form a loadedresin containing the removed valuable metal and a barren leach solutionfor recycle to the leaching operation. The loaded resin is contactedwith a stripping solution to dissolve at least most of the removedvaluable metal, forming a barren resin for recycle to the solventextraction step and a loaded stripping solution containing at least mostof the valuable metal. The dissolved valuable metals are separated fromthe loaded stripping solution, such as by precipitation, further solventextraction, or phase transfer extraction (such as, with anitrogen-containing phase transfer agent), to form a barren strippingsolution for recycle to the solvent extraction step and a separatedvaluable metal-containing material.

The cogen plant 120 provides power 170 to the pumps and other processequipment in the process plant 112 and waste heat 180, as needed, to theappropriate unit operations. In one configuration, the lixiviant and/orstripping solution include hydrochloric acid, and the above unitoperations in the process plant 112 produce a byproduct salt solution,which, in some applications, is an acidic brine solution. As noted, thissolution can be recycled to the primary and secondary treatment circuitsfor purification prior to introduction to the electrochemical acidgeneration unit to generate more acid 142 and other products 140. Theprimary and secondary treatment circuits treat the byproduct saltsolution, as noted above, to remove at least most of the polyvalentcations before introducing the treated or purified byproduct saltsolution to the electrochemical acid generation unit.

In the electrochemical acid generation plant 116, the byproduct saltsolution is converted, as noted above, into caustic soda, sodiumhypochlorite, hydrogen gas, and chlorine gas. The hydrogen gas andchlorine gas are thermally reacted to produce hydrochloric acid 142 forrecycle to the process plant 112. Because a portion of the hydrogen gasis lost and a substantial stoichiometric imbalance (see equations 1-6above) exists between hydrogen gas and chlorine gas, a portion of thechlorine gas can be used to manufacture bleach for sale. Alternatively,the chlorine gas can be sold for other applications, such as themanufacture of chlorinated solvents or chlorinated organics. In thismanner, an approximate stoichiometric balance between hydrogen andchlorine gas is maintained in the process. The cogen plant 120 providespower 170 and waste heat 180 (typically in the form of steam) to theappropriate unit operations in the electrochemical acid generation plant116. Byproduct water 128 from the plant 116 is recycled to the cogenplant 120, mill 108, and process plant 112.

With reference to FIG. 2, a second embodiment will now be discussed.

The valuable (acid soluble) metal-containing material 104 is milled inthe mill 108. In the mill, the material 104 is comminuted, by wet and/ordry crushers and grinding mills in an open or closed circuit, to producea comminuted material (not shown). The comminuted material is commonlyconcentrated, such as by flotation or size or weight separationtechniques, to produce a concentrate 200, which commonly is in the formof a slurry.

The concentrate (slurry) 200 is introduced into the process plant 112.In the process plant 112, the concentrate 220 is vat or heap leached(step 204), biologically and/or chemically, by a leach solution (notshown) comprising a mineral acid to dissolve at least most of thevaluable metal in the leach solution to form a pregnant leach solution208. The pregnant leach solution 208 is optionally separated (step 212)to produce a valuable metal-barren material 132, a valuable metal-barrensalt solution 216, and a valuable metal-rich solution 220. The valuablemetal-rich solution 220 includes at least most of the dissolved valuablemetal in the pregnant leach solution.

In one configuration, the separation includes a thickener/wash circuit,such as a counter current decantation circuit, to remove the solid-phasevaluable metal-barren material 132 from the valuable metal-rich liquidphase (not shown). As will be appreciated, other liquid/solid separationtechniques may be employed, such as filtration, screening, cyclones, andother size or weight separation techniques.

The valuable metal-rich liquid phase is then subjected to sorption (suchas using an ion exchange or chelating resin) or membrane filtration toremove at least most of the valuable metal from the liquid phase andform a valuable metal-barren leach solution for recycle to the valuablemetal dissolution step 204. The sorbent can be an ion exchange orchelating resin, a porous media (e.g., activated carbon, zeolites, andother porous media), and the like. While sorption and membraneseparation are discussed with reference to the removal of a selected ortarget valuable metal, it is to be understood that sorption and/ormembrane separation may also be used, in addition to or in lieu ofvaluable target metal sorption, in separation 212 to remove impurities,such as other valuable or invaluable metals, thereby purifying thetarget valuable metal-containing pregnant leach solution.

The sorbed target valuable metal is stripped from the sorbent (notshown) by a stripping solution (such as an eluant) by a change (relativeto the pregnant leach solution) in temperature and/or pH (which changesthe preference for the sorbent of the target valuable metal) to form atarget valuable metal-rich stripping solution (not shown) and strippedsorbent for recontact with the pregnant leach solution 208.

The target valuable metal-rich stripping solution is formed into atarget valuable metal product (not shown) (operation 136) and abyproduct salt solution 224. Valuable metal product formation can be,for example, by electrolysis or electrowinning, precipitation (which,for instance, forms a target metal sulfide or oxide), sorption (such asusing activated carbon), membrane filtration, cementation, and/oramalgamation.

In the mill 108 and process plant 112, there are a number of processesfor recovering rare earth metals as valuable metals.

One process configuration, that is particularly applicable tobastnaesite, selectively oxidizes rare earths. Cerium is separated afteroxidation of cerium (III) to cerium (IV), simplifying the subsequentseparation of the less abundant lanthanides. Oxidation occurs whenbastnaesite is heated in the presence of molecular oxygen at atemperature typically of at least about 500° C. and even more typicallyof at least about 600° C. or when rare earth hydroxides are dried in thepresence of molecular oxygen at a temperature, commonly in the range offrom about 120 to about 130° C. Cerium (IV) is separated from thetrivalent rare earths either by selective dissolution of trivalent rareearths with dilute acid or by complete dissolution of trivalent specieswith concentrated acid followed by selective precipitation of cerichydroxide or solvent extraction of cerium (IV) as noted below. Inaqueous solutions, cerium (III) is oxidized to cerium (IV) byelectrolysis or treatment with hydrogen peroxide or sodium hypochlorite.Precipitation of hydrated cerium oxide then occurs when the pH isadjusted commonly to a pH of at least about pH 3 and even more commonlyranging from about pH 3 to about pH 7.

Another process configuration for recovering rare earths is set forth inU.S. Pat. Nos. 5,207,995 and 5,433,931, each of which is incorporatedherein by this reference. The process is particularly useful inrecovering rare earths from bastnaesite. In the process, a rare earthore is ground to a P₉₀ size of 100 mesh (Tyler) (or a common mean,median, or P₉₀ size ranging from about 1 to about 100 microns and evenmore commonly from about 5 to about 25 microns). The ground ore isfloated to form a rare earth concentrate (comprising most of thebastnaesite in the rare earth ore with the quartz, barite, calcite, andstrontianite being separated in tailings). The concentrate is typicallyat least about 25 wt. % and even more typically ranges from about 35 toabout 75 wt. % rare earths. The concentrate is subjected to a first acidleach with dilute hydrochloric acid (pH about 1.0) to remove some of thealkaline earth constituents of the concentrate and the leached oreroasted. The roasting is typically at about 400° C. to about 800° C. inthe presence of molecular oxygen to convert fluorocarbonate mineral to amixture of fluorides and oxides and oxidize cerium to cerium (IV). Theroasted ore is subjected to a second acid leach with a more concentratedhydrochloric acid solution (which commonly comprises from about 0.1 toabout 0.5N to about 0.2N hydrochloric acid) to remove the remainingalkaline earth constituents and separate cerium from other rare earthoxides. The ore is then treated with a third acid leach with a stillmore concentrated hydrochloric acid solution (e.g., commonly at leastabout 25 wt. %, more commonly from about 35 to about 75 wt. %, and evenmore commonly from about 40 to about 50 wt. % hydrochloric acid) tosolubilize the cerium values for further processing. The pregnant leachsolution typically includes at least most of the rare earth content ofthe rare earth concentrate and even more typically includes from about25 to about 95 wt. % rare earths.

In another process configuration used for bastnaesite, the rare earthconcentrate is leached with diluted or concentrated hydrochloric acid todissolve, at least partially, the rare earths, which combine with thefluorine from the ore. The mixed rare earth-fluoride residue isdecomposed using caustic soda at a temperature commonly ranging fromabout 100 to about 300° C. The resulting rare earth hydroxides areleached with diluted or concentrated hydrochloric acid. In anotherversion of the process, diluted or concentrated sulfuric acid, insteadof hydrochloric acid, can be used to dissolve the residue at atemperature commonly ranging from about 200 to about 500° C. Thedissolved rare earths are then recovered as water-soluble sulfates.Polyvalent impurities, such as iron, are removed by pH neutralization.

In another process configuration, the rare earth is present in monaziteand recovered by industrial digestion using caustic soda. The phosphatecontent of the ore is recovered as trisodium phosphate and the rareearths as rare earth hydroxides. The lixiviant commonly contains fromabout 25 to about 75 wt. % sodium or potassium hydroxide solution at atemperature ranging from about 125 to about 200° C. The resultant mixedrare earth and thorium hydroxide precipitate is dissolved inhydrochloric and/or nitric acid, processed to remove at least most ofthe thorium and other non-rare earth elements, and processed to recoverthe individual rare earths.

In another process configuration, the rare earth is present in lopariteand recovered by a chlorination technique. This technique is conductedusing gaseous chlorine at a temperature commonly ranging from about 500to about 1,000° C. in the presence of carbon. Volatile chlorides areseparated from the calcium-sodium-rare earth fused chloride, and theresultant precipitate dissolved in water. The dissolved rare earths arerecovered by suitable techniques.

In another process configuration, the rare earth is present in lopariteand recovered by a sulfation technique. This technique is conductedusing a sulfuric acid solution (typically having from about 50 to about95 wt. % sulfuric acid) at a temperature ranging from about 100 to about250° C. in the presence of ammonium sulfate. The product is leached withwater, while the double sulfates of the rare earths remain in theresidue. The titanium, tantalum, and niobium sulfates transfer to thesolution. The residue is converted to rare earth carbonates and thendissolved in, and isolated by suitable techniques from, nitric acid.

In the above process configurations, the concentrated rare earths can berecovered by any of a number of different techniques. In oneconfiguration, the concentrated rare earths are separated by ionexchange. For example, pH dependent rare earth complexes form withcitric acid or aminopolycarboxylate eluants (e.g.,ethylenediaminetetraacetic acid (EDTA) andhydroxyethylenediaminetriacetic acid (HEEDTA). Phosphate-free resins arepreferred to avoid rare earth poisoning of the resin due to incompleteelution of the rare earth from the resin. The rare earths are recoveredby elution using a concentrated solution of a monovalent salt, such asammonium chloride or sodium chloride. If a complexing agent exhibitingsignificantly different affinities for the various lanthanides is addedto the eluant, a separation occurs. In another configuration,oil-soluble compounds separate rare earths by liquid-liquid extractionusing acidic, basic, and/or neutral extractants. Typical acidic, basic,and neutral extractants include carboxylic acids, organophosphorus acidsand esters thereof, tetraalkylammonium salts, alcohols, ethers, andketones. In another configuration, rare earth halides are reduced tometal by reaction of more electropositive metals, such as calcium,lithium, sodium, potassium, and aluminum. In another configuration,electrolytic reduction is used to produce light lanthanide metals,including didymium (a Nd—Pr mixture). In another configuration,fractional distillation is used to recover and separate rare earths. Inanother configuration, zone melting is used to recover and separate rareearths. Due to the highly electropositive nature of rare earths, rareearth metals can be formed from aqueous solutions by fused saltelectrolysis or metallothermic reduction.

The byproduct salt solution 224 and salt solution 216 can each include avariety of polyvalent impurities, including one or more of: more thanabout 20 ppb divalent calcium, more than about 20 ppb divalentmagnesium, more than about 100 ppb divalent strontium, more than about500 ppb divalent barium, more than about 100 ppb trivalent aluminum,more than about 1 ppm trivalent iron, more than about 15 ppm divalentmercury, more than about 10 g/L divalent sulfate anion, more than about10 ppm silica, more than about 400 ppb monovalent fluorine, more thanabout 100 ppm radioactive nuclides (e.g., radium, uranium, and thorium)and daughters thereof, and more than about 10 ppb divalent nickel. Someof the impurities can be present at relatively high concentrations up totheir solubility limits.

The byproduct salt solution 224 is combined with the salt solution 216,and the combined solution 228 optionally subjected to inorganiccontaminant purification (step 232) to form a first purified solution236. Although any contaminant removal techniques may be employed,inorganic contaminant removal can be by saturation, precipitation (suchas with sodium or potassium hydroxide, oxide, or carbonate),clarification, filtration (such as membrane filtration), sorption (suchas using an ion exchange or chelating resin (e.g., resins havingaminomethylphosphonic-, iminodiacetic-type, or thiol functional groups),activated carbon, zeolites, alumina, silica alumina, and the like),electrolysis, dechlorination, cementation, and amalgamation). In oneconfiguration, at least most of the dissolved polyvalent inorganicimpurities, such as calcium, magnesium, iron, and other impurities, areremoved by precipitation as oxides, carbonates, and/or hydroxides. Thisis typically effected using precipitants having a monovalent cation,such as sodium carbonate and sodium hydroxide. The precipitatedimpurities are removed or separated from the liquid phase by athickening circuit, screening, filtration, cyclones, and the like. Inone configuration, at least most of the dissolved polyvalent inorganicimpurities are removed by an ion exchange or chelating resin. When thevaluable metal is a rare earth, the resin should be substantially freeof phosphate groups to avoid rare earth “poisoning” of the resin byincomplete elution of the rare earth. In one configuration, sulfate andother polyvalent anions are removed by refrigeration andcrystallization, evaporative crystallization, and/or salting out of thecontaminant.

The first purified solution 236 is optionally subjected to organiccontaminant removal (step 240) to form a second purified solution 244.Although any contaminant removal techniques may be employed to remove atleast most of the organics from the first purified solution 236, organiccontaminant removal is commonly done by one or more of vacuumdistillation, perevaporation, steam stripping, sorption (such as usingan ion exchange or chelating resin), and membrane filtration.

The second purified solution 244 is optionally subjected to trace ionremoval (step 248) to remove at least most of any remaining polyvalentions and form a third purified solution 252. Step 248 is, in effect, apolishing operation. While any techniques (including those discussedabove with reference to step 232) may be employed to remove remainingpolyvalent ions, a common polishing mechanism is sorption (such as usingan ion exchange or chelating resin) of the remaining polyvalentinorganic impurities. The third purified solution 252 should have asatisfactory level of impurities for the particular type ofelectrochemical acid generation employed. In one configuration, thethird purified solution 252 has a salt at its saturation (under processoperating temperature and pressure), which is usually between about 23to about 28 wt. % salt dissolved in water.

FIG. 3 shows one particular configuration for purifying the combinedsolution 228 that is particularly applicable to rare earth metalrecovery processes.

In a first stage precipitation of impurities 304, a base, such ascaustic soda, is added to the combined solution 228, which typically hasa typical pH of no more than about pH 8, to increase the pH to a typicalpH of at least about pH 9. Certain of the polyvalent cationicimpurities, namely trivalent rare earths, divalent alkaline earthmetals, divalent strontium, divalent barium, divalent nickel, andtrivalent aluminum, form carbonate precipitates. Trivalent irontypically does not precipitate in the first precipitation stage.

In a second stage precipitation of impurities 308, a stronger base, suchas sodium hydroxide, is contacted with the combined solution 228 tofurther increase the pH to a typical pH of at least about pH 10 and evenmore typically at least about pH 11. More of the polyvalent cationicimpurities, namely trivalent rare earths, divalent alkaline earthmetals, divalent strontium, divalent barium, trivalent iron, divalentnickel, and trivalent aluminum, precipitate as hydroxides. After thefirst and second stages, typically at least most, even more typically atleast about 75%, and even more typically at least about 90% of thepolyvalent cations and anions are in the form of precipitates.

After the second precipitation stage 308, the combined salt solution 228is contacted with a coagulant and flocculent and subjected toliquid/solid separation in step 312 by a suitable technique. Suitabletechniques include size and/or weight separation techniques, such asfiltration, cycloning, gravity settling, decantation, thickening, andcombinations thereof, to remove commonly most, even more commonly atleast about 75%, and even more commonly at least about 95% of theprecipitates from the solution 228.

Following liquid/solid separation, the combined solution 228 may bepH-adjusted followed by contact, in step 316, of the pH-adjustedsolution with a sorbent to remove at least most of the organic matter.The sorbent commonly used is activated carbon. The organic mattercommonly includes dissolved solvent extraction or ion exchange resins,surfactants, flotation reagents (e.g., collectors and frothers),coagulants, and flocculants. In one application, the pH of the combinedsolution 228 is decreased by mineral acid addition to a pH commonly ofno more than about pH 8.

The solution 228 is then subjected in step 324 to ion exchange removalof at least most of any remaining trivalent and higher valency cations.The resin commonly used has an iminodiacetic-type functional group.

The solution 228 is then passed through a mixed bed of anion and cationexchange resins to remove at least most of any remaining divalentcations and polyvalent anions, such as sulfates (SO₄ ²⁻) and nitrates(NO₃ ²⁻). The cation-exchange resin commonly used has anaminomethylphosphonic functional group. Sulfate and nitrate ions arestrongly attracted to most strong-base anion-exchange resins. Exemplaryanion-exchange resins include polystyrene resins (e.g., AmberliteIRA-400, 402, 404, 900, and 996™ by Aldrich, Duolite A-101D™, IonacASB-1 or 2™ and Ionac SR-7™, and Lewatit OC-1950™), polyacrylic resins(e.g., Amberlite IRA-458 and 958™), pyridine resins (e.g., Reillex HPQ™,B-1™, and DP-1™), and styrene-divinylbenzene copolymers which haveeither been sulphonated to form strongly acidic cation-exchangers oraminated to form strongly basic or weakly basic anion-exchangers.

The ordering of the iminodiacetic-type oraminomethylphosphonic-functional group resins in the treatment trainenables removal of at least most of any remaining trivalent or highervalency cations by the iminodiacetic-type functional group beforeremoval of the divalent cations by the aminomethylphosphonic-functionalgroup. As noted, trivalent and higher valency cations, particularlytrivalent rare earths, can poison the aminomethylphosphonic-functionalgroup by incomplete elution of such cations.

Because a substantial portion, and in some cases at least most, of thefluorine in the combined solution 228 has not been removed by the priorpurification steps and because fluorine can damage platinum electrodesin the electrochemical acid generation system, typically at least mostand even more typically at least about 85% of the fluorine is removed instep 322 by a suitable technique. One technique is to remove fluorine bypassing the solution 228 through an aluminum oxide polishing column.Another technique is to remove fluorine by passing the solution 228through a rare earth-containing column. The column contains rareearth-containing particulates that can be supported or unsupported. Theparticulates contain primarily, on weight and molar bases, rare earthcompounds. A preferred rare earth particulate is composed, on weight andmolar bases, primarily of compounds of cerium (III), (IV), or a mixturethereof. Stated another way, the rare earth component of the rareearth-containing particulates is primarily cerium.

The solution 228 is finally passed through a polishing column to removeat least most of any remaining cations and form the third purifiedsolution 252. A common polishing column comprises zeolites.

In another configuration, the various separations are effected usingmembrane filters applied to the solution 228 before or after first andsecond stage precipitation 304 and 308. For example, following removalof precipitated impurities 312, the solution 228 is first passed througha microfiltration and/or ultrafiltration membrane to remove in a firstretentate at least most suspended and colloidal solids and organiccontaminants and form a first permeate comprising at least most of theinorganic ions, and the first permeate is passed through anultrafiltration, nanofiltration, and/or leaky reverse osmosis membraneto remove in a second retentate at least most of the polyvalent ions inthe solution 228 and pass in a second permeate at least most of themonovalent ions in the solution 228. The second permeate is thenoptionally subjected to polishing to remove at least most of anyremaining polyvalent ions and/or undesirable monovalent ions,particularly fluorine.

Regardless of the particular purification techniques employed, the thirdpurified solution 252 typically has no more than about 20 ppb divalentcalcium and magnesium, no more than about 100 ppb divalent strontium, nomore than about 500 ppb divalent barium, no more than about 100 ppbtrivalent aluminum, no more than about 1 ppm trivalent iron, no morethan about 15 ppm divalent mercury, no more than about 10 g/L divalentsulfate anion, no more than about 10 ppm silica (in the presence ofdivalent calcium and trivalent aluminum), no more than about 400 ppbmonovalent iodine (in the presence of divalent barium), and no more thanabout 10 ppb divalent nickel. In some applications, each impurity in thethird purified solution 252 is present at a concentration of no morethan about 1 ppm.

The above purification steps are typically performed to maintain atleast most, even more typically at least about 75%, and even moretypically at least about 95% of the salt cation and anion (e.g., sodiumion and chlorine ion) in solution. The various steps are thereforeselectively performed to remove polyvalent and organic contaminantswhile avoiding removal of the salt components. Stated another way, thecation and anion exchange resins and sorbents referenced above, underthe conditions of the solution 228, generally have limited or noaffinity for either sodium or chlorine ions (when the salt is sodiumchloride).

If necessary, the third purified solution 252 may be subjected to saltconcentration (step 256) to adjust the salinity of the solution 252 to alevel suitable for electrochemical acid generation. The saltconcentrator may include multiple effect evaporators, energy efficientvapor recompressors, recompressors, and combinations thereof. Ifnecessary, pH of the third purified solution 252 is performed using anacid or base produced by electrochemical acid generation operation 280.

The third purified solution 252 is introduced into the electrochemicalacid generation operation 280 to convert the salt into a desired mix ofthe end products referenced above. In the configuration of FIG. 2, theend products are an aqueous mineral acid solution 260 and an aqueoussodium hydroxide solution 264. The aqueous mineral acid solution 260 isdirected to the valuable metal dissolution operation 204. The aqueousbase solution 264 is directed to the separation and product formationoperations 212 and 136, as needed. Additional (fresh) salt solution 268,such as surface water, municipal water, industrial water, condensedsteam, sea water, brine, or synthetically produced saline water, isadded, as needed, to replace respective losses in the various unitoperations.

The acid and base solutions can be concentrated, by optionalconcentrators 278 and 272, respectively, to produce the desired acid orbase concentrations. Typically, the acid and base solutions will haveacid and base concentrations, respectively, of no more than about 90,even more typically no more than about 75, and even more typically nomore than about 50 wt. %. Exemplary concentrators are evaporators anddistillation columns. In some applications, the acid or base solutionsmay require dilution to yield appropriate concentration levels.

The base solution can be pH adjusted in operation 282 using a suitablepH adjuster, such as an acidic pH or basic pH adjustor, as needed.Typically, the basic pH adjustor is sodium or potassium hydroxideproduced during electrochemical acid generation 116.

Although not shown, additional hydrogen gas may need to be supplied tooffset hydrogen losses during the process.

Water balance in the process can be maintained by a multiple-effectevaporation step. This occurs at the point in the process circuit wherethe salt is likely to precipitate due to super-saturation. Theprecipitated salt may be recycled back to the electrochemical acidgeneration operation 280.

EXAMPLES Example A

Example A was a determination of a multi-stage precipitation and ionexchange process for removing divalent and trivalent cations prior to asalt splitting process. FIGS. 4 and 5, respectively, show decreases inthe divalent alkaline earth (specifically, magnesium, calcium, strontiumand barium) and trivalent (lanthanum, cerium, praseodymium, neodymium,samarium and iron) cations after each of the precipitation and ionexchange stages.

M1 is the first precipitation stage (FIG. 3) where a salt solution (suchas, the byproduct salt solution 224, the valuable metal-barren saltsolution 216 or the combination of thereof (combined solution 228) asdescribed above) having a pH of about pH 7 was contacted with a sodiumcarbonate solution having a pH of about pH 9.5 to form a metal carbonateslurry. Dissolving sodium carbonate in water with agitation formed thesodium carbonate solution. The metal carbonate slurry had metalcarbonate precipitates dispersed in salt water. The metal carbonatestypically precipitated are lanthanum carbonate, cerium carbonate,praseodymium carbonate, neodymium carbonate, samarium carbonate,magnesium carbonate, strontium carbonate, barium carbonate, calciumcarbonate, lead carbonate, uranium carbonate and aluminum carbonate.

M2 is the second precipitation stage (FIG. 3) where the metal carbonateslurry was contacted with a sodium hydroxide solution having about 8 wt% NaOH to further raise the pH to a pH of from about pH 11 to about pH2and to further precipitate as hydroxides any of the metals identifiedabove (such as lanthanum, cerium, praseodymium, neodymium, samarium,magnesium, strontium, barium, calcium, lead, uranium and aluminum)remaining in solution.

M3 is third precipitation stage (FIG. 3) where a coagulant, such as alum(Al₂(SO₄)₃), was contacted with the metal carbonates andhydroxides(hereafter referred to as metal solids). The contacting of thecoagulant with the metal solids flocculated and/or increased theparticle size of the metal solids, thereby increasing the efficiency ofseparating the metal solids from the solution liquid phase. The liquidphase contained NaCl, organics, and decreased amounts of the divalentand trivalent cations compared to the salt solution (FIGS. 4 and 5).Coagulation and flocculation in a high salt concentration solution isdifficult. However, it is preferred to substantially remove divalent andtrivalent ions and/or solids prior to conducting a chloroalkali process.Hydrochloric acid (about 18 wt % HCl) was added to the aqueous stream toadjust the pH to about pH7.

The pH adjusted aqueous stream was filtered and ran through an activatedcarbon filter prior to contacting the aqueous stream with a first IX1ion exchange resin IX1 (FIG. 3). The first ion exchange resin was animinodiacetic function resin sold under the trade name of AmberliteIRC-748i from Rohm & Haas to form a first ion-exchanged solution havinga decreased content of divalent and trivalent cations compared to the pHadjusted aqueous stream (FIGS. 4 and 5).

The first ion-exchanged solution was contacted with a secondion-exchange resin IX2 (FIG. 3) to form a second ion-exchanged solutionhaving a reduced divalent and trivalent ion content compared to thefirst ion-exchanged solution (FIGS. 4 and 5). The second ion-exchangeresin is an aminomethylphosphonic function resin sold under the tradename of Amberlite IRC-747 by Rohm & Haas.

Example B

Example B was a determination of the loading capacity of trivalentcation on a chelating ion exchange resin (IX1 in FIG. 3). The chelatingion exchange resin evaluated was an iminodiacetic resin sold under thetrade name of Amberlite IRC-748i from Rohm & Haas. The trivalent cationwas lanthanum. A lanthanum feed solution having a pH of about pH 4,about 50 g/L NaCl and 83 mg/L of lanthanum (as LaCl₃) was prepared bydissolving about 400 mg of Lanthanum oxide (La₂O₃) in hydrochloric acid(about 3.7 ml of 2 N HCl)). After dissolving the lanthanum oxide, about200 grams of NaCl was added, the pH was adjusted with 1 N NaOH to a pHof about pH 4 and de-ionized water was added to form a final volume ofabout 4 liters. A column was packed with the Amberlite IRC-748i resin.The lanthanum feed solution as passed through the packed column at arate of about 2.05 mL/min at about 21 degrees Celsius (see FIGS. 6). Themaximum trivalent cation capacity of the iminodiacetic resin wasdetermined to be about 117 mg of lanthanum or about 29 mg of lanthanumper gram of resin. The resin was loaded with about 108 mg of lanthanum.The total loading was calculated by determining the area under thebreakthrough curve (FIG. 6).

Example C

Example C was a determination of the removal capacity of the trivalentcation loaded on the resin in IX1 in Example B. The resin tested was animinodiacetic function resin sold under the tradename of AmberliteIRC-748i by Rohm & Haas. The trivalent cation was lanthanum. About 108milligrams of lanthanum was loaded on a resin column containing about 4grams of Amberlite 748i. The lanthanum loaded column was regeneratedwith a hydrochloric acid solution having a normality of about 2.6N, theflow rate of the hydrochloric acid solution was about 2.7 mL/min.Fractions were collected about every 5 minutes. The first 5 fractionscontained detectable amounts of lanthanum (see FIG. 7). The first 5fractions contained a total of 104 mg of lanthanum, which was withinexperimental error of the 108 mg of lanthanum loaded on the column. Thesecond fraction had the highest lanthanum concentration of about 7.5g/L. The fractions beyond the fifth fraction did not contain anydetectable amounts of lanthanum. It was assumed from this example thatan iminodiacetic function resin loaded with a trivalent cation, such aslanthanum, can be regenerated with hydrochloric acid.

Example D

Example D was a determination of the removal capacity of a trivalentcation loaded on a resin in IX2 of the brine finishing process (FIG. 3).The resin tested was an aminomethylphosphonic function resin sold underthe trade name of Amberlite IRC-747 by Rohm & Haas. The trivalent cationwas lanthanum. About 88 mg of lanthanum was loaded on a resin columncontaining about 4 grams of Amberlite IRC-747. The loaded column wasregenerated with a hydrochloric acid solution having a normality ofabout 2.6 N. The flow rate of the 2.6 N HCl solution was about 1.9mL/min. 20 volume fractions were collected from the column. Fractionswere collected about every 5 minutes. Lanthanum was detected in each ofthe twenty volume fractions. While about 88 mg of lanthanum appeared tohave been loaded on the column, about 117 mg of lanthanum appeared tohave been unloaded from the column (FIG. 8). This discrepancy wasbelieved to be due to an analytical error. More specifically, it isbelieved that the column was loaded with a feed solution containing 60mg lanthanum/L and not about 42 mg lanthanum/L. About 125 mg oflanthanum would have been loaded on the column from the 60 mglanthanum/L solution, which would have better coincided with the 117 mgof lanthanum unloaded from the column.

Example E

Example E was a determination of optimal operating conditions for saltsplitting prior to operating the salt splitter in a steady state,continuous mode. Inductively coupled plasma atomic emission spectroscopy(ICP-AES) was used to verify the purity of the brine feed. The brinefeed had no more than about 0.5 ppm of divalents and iron. Salinity ofthe feed tank was measured with a conductivity probe and found to beabout 7.8 mmhos. The conductivity probe was calibrated against 3calibration standards at 5, 50 and 100 g/L salt, which hadconductivities of 0.82, 6.84 and 13.21 mmhos, respectively. Current andvoltage levels were read from salt splitter DC-power supply. The brinefeed solution was circulated through a bipolar membrane electrodialysisstack, that is an anion exchange membrane, cation exchange membrane andbipolar membrane, gaskets, flow distribution, electrodes, etc at about0.8 gallons per minute. This circulation rate turned each of the saltwater feed, acid, base and electrode rinse tanks, respectively, havingabout 12 liters of solution, over about every 4 minutes. The acid andbase salt splitter tanks contained de-ionized water. The electrode rinsetank contained 2N NaOH solution and the brine feed solution containedabout 75 g NaCl/liter and had a pH of about pH 2. After a consistentflow rate was established through the membrane stack and a solutionsubstantially free of bubbles was obtained, the DC power supply wasactivated. The DC power supply was adjusted to pass about 16 amps ofcurrent through the brine solution, while the voltage was allowed tovary. The conductivity, current, voltage, feed solution temperature andacid and base normalities were determined as a function of time untilthe brine feed NaCl content was substantially depleted to about zero(FIG. 9). The NaCl content of the brine feed was depleted in about 3.5hours. The acid and base compartments, respectively, had endingnormalities of about 0.8 N HCl and about 0.8 N NaOH.

Example F

Example F was a determination of the conversion rate for a salt feedcontaining about 95 grams NaCl per liter. The brine feed was verifiedfor purity using ICP-AES. The brine feed had no more than about 0.5 ppmof divalents and iron. Salinity of the feed tank was measured with aconductivity probe and found to be about 7.8 mmhos. The conductivityprobe was calibrated against 3 calibration standards at 5, 50 and 100g/L salt, which had conductivities of 0.82, 6.84 and 13.21 mmhos,respectively. Current and voltage levels were read from the saltsplitter DC-power supply. The brine feed solution was circulated througha bipolar membrane electrodialysis stack at about 0.8 gallons perminute. This circulation rate turned each of the salt water feed, acid,base and electrode rinse tanks, respectively, having about 12 liters ofsolution over about every 4 minutes. The acid and base salt splittertanks, respectively, contained about 0.5 N HCl and about 0.5 N NaOH. Theelectrode rinse tank contained a 2N NaOH solution and the brine feedtank contained about 95 g NaCl/liter and had a pH of about pH2. The DCpower supply was activated after a consistent flow rate was establishedthrough the membrane stack and the solution was substantially free ofbubbles. The DC power supply was adjusted to pass about 16 amps ofcurrent through the brine solution and the voltage was allowed to vary.After about 30 minutes of operation, the applied voltage and currentstabilized to about 19 volts and 16 amps, respectively (FIG. 10). Theconductivity, current, voltage, feed solution temperature and acid andbase normalities were measured as a function of time (FIG. 10). The NaClcontent of the brine feed decreased during electrolysis, from about 95g/L to about 17 g/L over about a 5 hour electrolysis period. Further,over the 5 hour electrolysis period, about 934 grams of NaCl wasconverted into hydrochloric acid and sodium hydroxide. The averageconversion rate was about 22 grams per square meter (of electrodesurface area) per minute. The acid and base compartments, respectively,had ending normalities of about 2 N HCl and about 2 N NaOH. About 800grams of water was electrolyzed in the process. A quantitative analysisof the amount of NaCl in the feed solution consumed per hour byelectrolysis yielded the following quadratic equation:

C_(i)[g/L]−2.34t²−1.76t+95.81, where t is hours

The DC power supply, on average, applied about 16 amps at about a 19volt potential. The theoretical equivalents of NaOH and HCl producedwere determined to be about 4.2 equivalents per hour, with a currentefficiency of about 76%. The power utilized to convert NaCl tohydrochloric and sodium hydroxide was about 1.6 kW hours per kg of NaClproduced.

A number of variations and modifications can be used. It would bepossible to provide for some features without providing others.

The various aspects, embodiments, and configurations, includecomponents, methods, processes, systems and/or apparatus substantiallyas depicted and described herein, including various embodiments,configurations, aspects, subcombinations, and subsets thereof. Those ofskill in the art will understand how to make and use the aspects,embodiments, or configurations disclosed herein after understanding thepresent disclosure. The various aspects, embodiments, andconfigurations, include providing devices and processes in the absenceof items not depicted and/or described herein or in various embodiments,configurations, or aspects hereof, including in the absence of suchitems as may have been used in previous devices or processes, e.g., forimproving performance, achieving ease and\or reducing cost ofimplementation.

The foregoing discussion has been presented for purposes of illustrationand description. The foregoing is not intended to limit the aspects,embodiments, or configurations to the form or forms disclosed herein. Inthe foregoing Detailed Description for example, various features of theaspects, embodiments, or configurations are grouped together in one ormore embodiments, configurations, or aspects for the purpose ofstreamlining the disclosure. The features of the aspects, embodiments,or configurations, may be combined in alternate aspects, embodiments, orconfigurations other than those discussed above. This method ofdisclosure is not to be interpreted as reflecting an intention that theaspects, embodiments, or configurations require more features than areexpressly recited in each claim. Rather, as the following claimsreflect, inventive aspects lie in less than all features of a singleforegoing disclosed embodiment, configuration, or aspect. Thus, thefollowing claims are hereby incorporated into this Detailed Description,with each claim standing on its own as a separate aspect, embodiment, orconfiguration.

Moreover, though the description has included description of one or moreaspects, embodiments, or configurations and certain variations andmodifications, other variations, combinations, and modifications arewithin the scope of the aspects, embodiments, or configurations, e.g.,as may be within the skill and knowledge of those in the art, afterunderstanding the present disclosure. It is intended to obtain rightswhich include alternative embodiments, configurations, or aspects to theextent permitted, including alternate, interchangeable and/or equivalentstructures, functions, ranges or steps to those claimed, whether or notsuch alternate, interchangeable and/or equivalent structures, functions,ranges or steps are disclosed herein, and without intending to publiclydedicate any patentable subject matter.

What is claimed is:
 1. A process, comprising: (a) contacting a valuablemetal-containing material with an acidic leaching solution to form apregnant leach solution comprising a dissolved valuable metal; (b)recovering the dissolved valuable metal to form a valuable metal productand a byproduct salt solution derived from reaction of an acid componentof the leaching solution with a base; (c) converting, by at least one ofa chloralkali and bipolar membrane electrodialysis cell, the byproductsalt solution into the acid component and the base; (d) recycling theacid component, as part of the acidic leaching solution, to step (a);and (e) recycling the base to at least one of steps (a) and (b).
 2. Theprocess of claim 1, wherein at least most of the byproduct salt solutionis converted into the acid component and base and wherein at least mostof the acid component and base are recycled.
 3. The process of claim 1,wherein the valuable metal is a rare earth, wherein the acid componentis hydrochloric acid, wherein the salt in the byproduct salt solution isone or more of sodium chloride and potassium chloride, wherein the baseis one or more of sodium hydroxide and potassium hydroxide, and whereinthe valuable metal product is a rare earth oxide.
 4. The process ofclaim 1, wherein the at least one of a chloralkali and bipolar membraneelectrodialysis cell is the bipolar membrane electrodialysis cell,wherein the valuable metal is one or more of copper, beryllium, nickel,iron, lead, molybdenum, and manganese, wherein the acid component isnitric acid, wherein the salt in the byproduct salt solution is one ormore of sodium nitrate and potassium nitrate, and wherein the base isone or more of sodium and potassium hydroxide.
 5. The process of claim1, wherein the at least one of a chloralkali and bipolar membraneelectrodialysis cell is the bipolar membrane electrodialysis cell,wherein the valuable metal is uranium, wherein the acid component isphosphoric acid, wherein the salt in the byproduct salt solution is oneor more of sodium phosphate and potassium phosphate, and wherein thebase is one or more of sodium and potassium hydroxide.
 6. The process ofclaim 1, wherein the at least one of a chloralkali and bipolar membraneelectrodialysis cell is the bipolar membrane electrodialysis cell,wherein the valuable metal is one or more of a platinum group metal,copper, beryllium, nickel, iron, lead, molybdenum, aluminum, germanium,uranium, gold, silver, cobalt, zinc, cobalt, tin, titanium, chromium,and manganese, wherein the salt in the byproduct salt solution is one ormore of sodium sulfate and potassium sulfate, wherein the acid componentis sulfuric acid, and wherein the base is one or more of sodium andpotassium hydroxide.
 7. The process of claim 1, wherein the valuablemetal is one or more of yttrium, scandium, a lanthanide, a platinumgroup metal, copper, chromium, beryllium, nickel, iron, lead,molybdenum, aluminum, germanium, uranium, gold, silver, cobalt, zinc,cobalt, tin, titanium, and manganese, wherein the salt in the byproductsalt solution is one or more of sodium chloride and potassium chloride,wherein the acid component is hydrochloric acid, and wherein the base isone or more of sodium and potassium hydroxide.
 8. The process of claim1, wherein the acid component is hydrochloric acid, wherein theconverting step produces hydrogen gas and chlorine gas, and wherein theconverting step further comprises: reacting chlorine gas with hydrogengas to produce hydrochloric acid.
 9. The process of claim 1, wherein theconverting step comprises: removing at least most of a selectedpolyvalent impurity from the byproduct salt solution to form a purifiedsalt solution; and introducing the purified salt solution into the atleast one of a chloralkali and bipolar membrane electrodialysis cell toform the acid component and base.
 10. The process of claim 9, whereinthe selected polyvalent impurity is a cation, wherein the selectedpolyvalent cation is removed by precipitation induced by a pH changeresulting from contact of the base with the byproduct salt solution, andwherein the introducing step comprises: contacting the purified saltsolution with an ion exchange resin to remove additional polyvalentcationic impurities; thereafter processing the purified salt solution bya salt concentrator to form a concentrated and purified salt solution;and introducing a concentrated and purified solution and a mineral acidinto an anolyte recirculation tank, wherein the concentrated andpurified solution is introduced into the at least one of a chloralkaliand bipolar membrane electrodialysis cell.
 11. The process of claim 1,further comprising: receiving electrical energy from a cogen plant, theelectrical energy being used in one or more of the contacting,recovering, converting and recycling steps; receiving waste heat fromthe cogen plant, the waste heat being used in one or more of thecontacting, recovering, converting and recycling steps.
 12. The processof claim 1, further comprising: maintaining an approximatestoichiometric balance between chlorine and hydrogen gas produced in theconverting step.
 13. The process of claim 1, wherein the byproduct saltsolution comprises an organic contaminant and wherein the convertingstep comprises: removing at least most of the organic contaminant toform a purified salt solution, wherein the purified salt solution isintroduced into the at least one of a chloralkali and bipolar membraneelectrodialysis cell to form the acid component and base.
 14. Theprocess of claim 1, wherein, in each of the recycle steps, the acidcomponent and base are concentrated and/or pH adjusted.
 15. A valuablemetal product recovered by the process of claim
 1. 16. A facility,comprising: (a) a mill to at least one of comminute a feed materialcomprising a valuable metal-containing mineral and form, from thevaluable metal-containing mineral, a concentrate containing the valuablemetal-containing mineral; (b) a process plant to recover the valuablemetal from the valuable metal-containing mineral, wherein at least oneof the mill and process plant generate a byproduct salt solution from amineral acid and a base; and (c) an electrochemical acid generationplant comprising at least one of a chloralkali and bipolar membraneelectrodialysis cell to generate the mineral acid and base from thebyproduct salt solution and provide the mineral acid to at least one ofthe mill and process plant.
 17. The facility of claim 16, wherein thevaluable metal is a rare earth, wherein the acid component ishydrochloric acid, wherein the salt in the byproduct salt solution isone or more of sodium chloride and potassium chloride, wherein the baseis one or more of sodium hydroxide and potassium hydroxide, and whereinthe valuable metal product is a rare earth oxide.
 18. The facility ofclaim 16, wherein the at least one of a chloralkali and bipolar membraneelectrodialysis cell is the bipolar membrane electrodialysis cell,wherein the valuable metal is one or more of copper, beryllium, nickel,iron, lead, molybdenum, and manganese, wherein the acid component isnitric acid, wherein the salt in the byproduct salt solution is one ormore of sodium nitrate and potassium nitrate, and wherein the base isone or more of sodium and potassium hydroxide.
 19. The facility of claim16, wherein the at least one of a chloralkali and bipolar membraneelectrodialysis cell is the bipolar membrane electrodialysis cell,wherein the valuable metal is uranium, wherein the acid component isphosphoric acid, wherein the salt in the byproduct salt solution is oneor more of sodium phosphate and potassium phosphate, and wherein thebase is one or more of sodium and potassium hydroxide.
 20. The facilityof claim 16, wherein the at least one of a chloralkali and bipolarmembrane electrodialysis cell is the bipolar membrane electrodialysiscell, wherein the valuable metal is one or more of a platinum groupmetal, copper, beryllium, nickel, iron, lead, molybdenum, aluminum,germanium, uranium, gold, silver, cobalt, zinc, cobalt, tin, titanium,chromium, and manganese, wherein the salt in the byproduct salt solutionis one or more of sodium sulfate and potassium sulfate, wherein the acidcomponent is sulfuric acid, and wherein the base is one or more ofsodium and potassium hydroxide. 21-52. (canceled)